(Polar molecules, Non-polar molecules, etc.)
6 posts • Page 1 of 1
Once you find the shape of a compound and determine if the compound is polar or non-polar how does this affect our analysis of the compound's boiling point. In other words, how do shape and polarity play into a compounds boiling point?
If a molecule is polar, it is able to form dipole-dipole intermolecular forces (and possibly hydrogen bonds) in addition to London Dispersion forces. With more forces and bonds, a molecule becomes harder to break, thus causing a higher boiling point to break the bonds and denature the molecule.
When looking at the Lewis Structure of the molecule, you can see if that molecule has single, double, or triple bonds. Depending on that, you can see how tightly bound the atoms are to the central atom. The higher the bond strength, the harder it is to break the bonds apart or leading to a higher boiling point. In terms of polarity, a molecule that is more polar will have a higher boiling point.
I believe that if the molecule is polar then it has a higher boiling point than something that is non-polar. But when comparing 2 polar molecules' boiling points it is important to recognize what forces are present (hydrogen bonding, LFD, Dipole-dipole) and the one with more forces present has a higher boiling point.
Polar molecules that can form strong intermolecular bonds, i.e. dipole-dipole/hydrogen bonds, or dipole-induced dipole bonds, tend to have higher boiling points and depending on the polar end of the molecule, it would determine the relative strength between the two molecules. On the other hand, nonpolar molecules depend on van der waal forces for intermolecular bonds, which in most cases are the weakest (however the more van der waal forces you have, the stronger the attractive forces; cumulative force).
Ion bond > H bond > dipole dipole > dipole induced > induced induced
Who is online
Users browsing this forum: No registered users and 2 guests